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**Collision theory** is a principle of chemistry used to predict the rates of chemical reactions. It states that when suitable particles of the reactant hit each other with the correct orientation, only a certain amount of collisions result in a perceptible or notable change; these successful changes are called successful collisions. The successful collisions must have enough energy, also known as activation energy, at the moment of impact to break the pre-existing bonds and form all new bonds. This results in the products of the reaction. The activation energy is often predicted using the Transition state theory. Increasing the concentration of the reactant brings about more collisions and hence more successful collisions. Increasing the temperature increases the average kinetic energy of the molecules in a solution, increasing the number of collisions that have enough energy. Collision theory was proposed independently by Max Trautz in 1916^{[1]} and William Lewis in 1918.^{[2]} ^{[3]}

When a catalyst is involved in the collision between the reactant molecules, less energy is required for the chemical change to take place, and hence more collisions have sufficient energy for the reaction to occur. The reaction rate therefore increases.

Collision theory is closely related to chemical kinetics.

Collision theory was initially developed for the gas reaction system with no dilution. But most reactions involve solutions, for example, gas reactions in a carrying inert gas, and almost all reactions in solutions. The collision frequency of the solute molecules in these solutions is now controlled by diffusion or Brownian motion of individual molecules. The flux of the diffusive molecules follows Fick's laws of diffusion. For particles in a solution, an example model to calculate the collision frequency and associated coagulation rate is the Smoluchowski coagulation equation proposed by Marian Smoluchowski in a seminal 1916 publication.^{[4]} In this model, Fick's flux at the infinite time limit is used to mimic the particle speed of the collision theory. Jixin Chen proposed a finite-time solution to the diffusion flux in 2022 which significantly changes the estimated collision frequency of two particles in a solution.^{[5]}

The rate for a bimolecular gas-phase reaction, A + B → product, predicted by collision theory is^{[6]}

where:

*k*is the rate constant in units of (number of molecules)^{−1}⋅s^{−1}⋅m^{3}.*n*_{A}is the number density of A in the gas in units of m^{−3}.*n*_{B}is the number density of B in the gas in units of m^{−3}. E.g. for a gas mixture with gas A concentration 0.1 mol⋅L^{−1}and B concentration 0.2 mol⋅L^{−1}, the number of density of A is 0.1×6.02×10^{23}÷10^{−3}= 6.02×10^{25}m^{−3}, the number of density of B is 0.2×6.02×10^{23}÷10^{−3}= 1.2×10^{26}m^{−3}*Z*is the collision frequency in units of m^{−3}⋅s^{−1}.- is the steric factor.
^{[7]} *E*_{a}is the activation energy of the reaction, in units of J⋅mol^{−1}.*T*is the temperature in units of K.*R*is the gas constant in units of J mol^{−1}K^{−1}.

The unit of *r*(*T*) can be converted to mol⋅L^{−1}⋅s^{−1}, after divided by (1000×*N*_{A}), where *N*_{A} is the Avogadro constant.

For a reaction between A and B, the collision frequency calculated with the hard-sphere model with the unit number of collisions per m^{3} per second is:

where:

*n*_{A}is the number density of A in the gas in units of m^{−3}.*n*_{B}is the number density of B in the gas in units of m^{−3}. E.g. for a gas mixture with gas A concentration 0.1 mol⋅L^{−1}and B concentration 0.2 mol⋅L^{−1}, the number of density of A is 0.1×6.02×10^{23}÷10^{−3}= 6.02×10^{25}m^{−3}, the number of density of B is 0.2×6.02×10^{23}÷10^{−3}= 1.2×10^{26}m^{−3}.*σ*_{AB}is the reaction cross section (unit m^{2}), the area when two molecules collide with each other, simplified to , where*r*_{A}the radius of A and*r*_{B}the radius of B in unit m.*k*_{B}is the Boltzmann constant unit J⋅K^{−1}.*T*is the absolute temperature (unit K).*μ*is the reduced mass of the reactants A and B, (unit kg)._{AB}*N*_{A}is the Avogadro constant.- [A] is molar concentration of A in unit mol⋅L
^{−1}. - [B] is molar concentration of B in unit mol⋅L
^{−1}. - Z can be converted to mole collision per liter per second dividing by 1000
*N*_{A}.

If all the units that are related to dimension are converted to dm, i.e. mol⋅dm^{−3} for [A] and [B], dm^{2} for *σ*_{AB}, dm^{2}⋅kg⋅s^{−2}⋅K^{−1} for the Boltzmann constant, then

unit mol⋅dm^{−3}⋅s^{−1}.

Consider the bimolecular elementary reaction:

- A + B → C

In collision theory it is considered that two particles A and B will collide if their nuclei get closer than a certain distance. The area around a molecule A in which it can collide with an approaching B molecule is called the cross section (σ_{AB}) of the reaction and is, in simplified terms, the area corresponding to a circle whose radius ( ) is the sum of the radii of both reacting molecules, which are supposed to be spherical.
A moving molecule will therefore sweep a volume per second as it moves, where is the average velocity of the particle. (This solely represents the classical notion of a collision of solid balls. As molecules are quantum-mechanical many-particle systems of electrons and nuclei based upon the Coulomb and exchange interactions, generally they neither obey rotational symmetry nor do they have a box potential. Therefore, more generally the cross section is defined as the reaction probability of a ray of A particles per areal density of B targets, which makes the definition independent from the nature of the interaction between A and B. Consequently, the radius is related to the length scale of their interaction potential.)

From kinetic theory it is known that a molecule of A has an average velocity (different from root mean square velocity) of , where is the Boltzmann constant, and is the mass of the molecule.

The solution of the two-body problem states that two different moving bodies can be treated as one body which has the reduced mass of both and moves with the velocity of the center of mass, so, in this system must be used instead of . Thus, for a given molecule A, it travels before hitting a molecule B if all B is fixed with no movement, where is the average traveling distance. Since B also moves, the relative velocity can be calculated using the reduced mass of A and B.

Therefore, the total **collision frequency**,^{[8]} of all A molecules, with all B molecules, is

From Maxwell–Boltzmann distribution it can be deduced that the fraction of collisions with more energy than the activation energy is . Therefore, the rate of a bimolecular reaction for ideal gases will be

- in unit number of molecular reactions s
^{−1}⋅m^{−3},

where:

*Z*is the collision frequency with unit s^{−1}⋅m^{−3}. The*z*is*Z*without [A][B].- is the steric factor, which will be discussed in detail in the next section,
*E*is the activation energy (per mole) of the reaction in unit J/mol,_{a}*T*is the absolute temperature in unit K,*R*is the gas constant in unit J/mol/K.- [A] is molar concentration of A in unit mol/L,
- [B] is molar concentration of B in unit mol/L.

The product *zρ* is equivalent to the preexponential factor of the Arrhenius equation.

Once a theory is formulated, its validity must be tested, that is, compare its predictions with the results of the experiments.

When the expression form of the rate constant is compared with the rate equation for an elementary bimolecular reaction, , it is noticed that

unit M^{−1}⋅s^{−1} (= dm^{3}⋅mol^{−1}⋅s^{−1}), with all dimension unit dm including *k*_{B}.

This expression is similar to the Arrhenius equation and gives the first theoretical explanation for the Arrhenius equation on a molecular basis. The weak temperature dependence of the preexponential factor is so small compared to the exponential factor that it cannot be measured experimentally, that is, "it is not feasible to establish, on the basis of temperature studies of the rate constant, whether the predicted *T*^{.mw-parser-output .sfrac{white-space:nowrap}.mw-parser-output .sfrac.tion,.mw-parser-output .sfrac .tion{display:inline-block;vertical-align:-0.5em;font-size:85%;text-align:center}.mw-parser-output .sfrac .num{display:block;line-height:1em;margin:0.0em 0.1em;border-bottom:1px solid}.mw-parser-output .sfrac .den{display:block;line-height:1em;margin:0.1em 0.1em}.mw-parser-output .sr-only{border:0;clip:rect(0,0,0,0);clip-path:polygon(0px 0px,0px 0px,0px 0px);height:1px;margin:-1px;overflow:hidden;padding:0;position:absolute;width:1px}1/2} dependence of the preexponential factor is observed experimentally".^{[9]}

If the values of the predicted rate constants are compared with the values of known rate constants, it is noticed that collision theory fails to estimate the constants correctly, and the more complex the molecules are, the more it fails. The reason for this is that particles have been supposed to be spherical and able to react in all directions, which is not true, as the orientation of the collisions is not always proper for the reaction. For example, in the hydrogenation reaction of ethylene the H_{2} molecule must approach the bonding zone between the atoms, and only a few of all the possible collisions fulfill this requirement.

To alleviate this problem, a new concept must be introduced: the **steric factor** *ρ*. It is defined as the ratio between the experimental value and the predicted one (or the ratio between the frequency factor and the collision frequency):

and it is most often less than unity.^{[7]}

Usually, the more complex the reactant molecules, the lower the steric factor. Nevertheless, some reactions exhibit steric factors greater than unity: the harpoon reactions, which involve atoms that exchange electrons, producing ions. The deviation from unity can have different causes: the molecules are not spherical, so different geometries are possible; not all the kinetic energy is delivered into the right spot; the presence of a solvent (when applied to solutions), etc.

Experimental rate constants compared to the ones predicted by collision theory for gas phase reactions Reaction *A*, s^{−1}M^{−1}*Z*, s^{−1}M^{−1}Steric factor 2ClNO → 2Cl + 2NO 9.4×10 ^{9}5.9×10 ^{10}0.16 2ClO → Cl _{2}+ O_{2}6.3×10 ^{7}2.5×10 ^{10}2.3×10 ^{−3}H _{2}+ C_{2}H_{4}→ C_{2}H_{6}1.24×10 ^{6}7.3×10 ^{11}1.7×10 ^{−6}Br _{2}+ K → KBr + Br1.0×10 ^{12}2.1×10 ^{11}4.3

Collision theory can be applied to reactions in solution; in that case, the *solvent cage* has an effect on the reactant molecules, and several collisions can take place in a single encounter, which leads to predicted preexponential factors being too large. *ρ* values greater than unity can be attributed to favorable entropic contributions.

Experimental rate constants compared to the ones predicted by collision theory for reactions in solution ^{[10]}Reaction Solvent *A*, 10^{11}s^{−1}⋅M^{−1}*Z*, 10^{11}s^{−1}⋅M^{−1}Steric factor C _{2}H_{5}Br + OH^{−}ethanol 4.30 3.86 1.11 C _{2}H_{5}O^{−}+ CH_{3}Iethanol 2.42 1.93 1.25 ClCH _{2}CO_{2}^{−}+ OH^{−}water 4.55 2.86 1.59 C _{3}H_{6}Br_{2}+ I^{−}methanol 1.07 1.39 0.77 HOCH _{2}CH_{2}Cl + OH^{−}water 25.5 2.78 9.17 4-CH _{3}C_{6}H_{4}O^{−}+ CH_{3}Iethanol 8.49 1.99 4.27 CH _{3}(CH_{2})_{2}Cl + I^{−}acetone 0.085 1.57 0.054 C _{5}H_{5}N + CH_{3}IC _{2}H_{2}Cl_{4}— — 2.0 10×10 ^{−6}

Collision in diluted gas or liquid solution is regulated by diffusion instead of direct collisions, which can be calculated from Fick's laws of diffusion. Theoretical models to calculate the collision frequency in solutions have been proposed by Marian Smoluchowski in a seminal 1916 publication at the infinite time limit,^{[4]} and Jixin Chen in 2022 at a finite-time approximation.^{[5]} A scheme of comparing the rate equations in pure gas and solution is shown in the right figure.

For a diluted solution in the gas or the liquid phase, the collision equation developed for neat gas is not suitable when diffusion takes control of the collision frequency, i.e., the direct collision between the two molecules no longer dominates. For any given molecule A, it has to collide with a lot of solvent molecules, let's say molecule C, before finding the B molecule to react with. Thus the probability of collision should be calculated using the Brownian motion model, which can be approximated to a diffusive flux using various boundary conditions that yield different equations in the Smoluchowski model and the JChen Model.

For the diffusive collision, at the infinite time limit when the molecular flux can be calculated from the Fick's laws of diffusion, in 1916 Smoluchowski derived a collision frequency between molecule A and B in a diluted solution:^{[4]}

where:

- is the collision frequency, unit #collisions/s in 1 m
^{3}of solution. - is the radius of the collision cross-section, unit m.
- is the relative diffusion constant between A and B, unit m
^{2}/s, and . - and are the number concentrations of molecules A and B in the solution respectively, unit #molecule/m
^{3}.

or

where:

- is in unit mole collisions/s in 1 L of solution.
- is the Avogadro constant.
- is the radius of the collision cross-section, unit m.
- is the relative diffusion constant between A and B, unit m
^{2}/s. - and are the molar concentrations of A and B respectively, unit mol/L.
- is the diffusive collision rate constant, unit L mol
^{−1}s^{−1}.

There have been a lot of extensions and modifications to the Smoluchowski model since it was proposed in 1916.

In 2022, Chen rationales that because the diffusive flux is evolving over time and the distance between the molecules has a finite value at a given concentration, there should be a critical time to cut off the evolution of the flux that will give a value much larger than the infinite solution Smoluchowski has proposed.^{[5]} So he proposes to use the average time for two molecules to switch places in the solution as the critical cut-off time, i.e., first neighbor visiting time. Although an alternative time could be the mean free path time or the average first passenger time, it overestimates the concentration gradient between the original location of the first passenger to the target. This hypothesis yields a fractal reaction kinetic rate equation of diffusive collision in a diluted solution:^{[5]}

where:

- is in unit mole collisions/s in 1 L of solution.
- is the Avogadro constant.
- is the area of the collision cross-section in unit m
^{2}. - is the product of the unitless fractions of reactive surface area on A and B. is the effective adsorption cross-section area.
- is the relative diffusion constant between A and B, unit m
^{2}/s, and . - and are the molar concentrations of A and B respectively, unit mol/L.
- is the diffusive collision rate constant, unit L
^{4/3}mol^{-4/3}s^{−1}.

**^**Trautz, Max.*Das Gesetz der Reaktionsgeschwindigkeit und der Gleichgewichte in Gasen. Bestätigung der Additivität von C*, Zeitschrift für anorganische und allgemeine Chemie, Volume 96, Issue 1, Pages 1–28, (1916)._{v}− 3/2 R. Neue Bestimmung der Integrationskonstanten und der Moleküldurchmesser**^**IUPAC,*Compendium of Chemical Terminology*, 2nd ed. (the "Gold Book") (1997). Online corrected version: (2006–) "collision theory". doi:10.1351/goldbook.C01170**^**William Cudmore McCullagh Lewis,*XLI.—Studies in catalysis. Part IX. The calculation in absolute measure of velocity constants and equilibrium constants in gaseous systems*, J. Chem. Soc., Trans., 1918, 113, 471-492.- ^
^{a}^{b}^{c}Smoluchowski, Marian (1916). "Drei Vorträge über Diffusion, Brownsche Molekularbewegung und Koagulation von Kolloidteilchen".*Phys. Z.*(in German).**17**: 557–571, 585–599. Bibcode:1916ZPhy...17..557S. - ^
^{a}^{b}^{c}^{d}Chen, Jixin (2022). "Why Should the Reaction Order of a Bimolecular Reaction be 2.33 Instead of 2?".*J. Phys. Chem. A*.**126**: 9719–9725. doi:10.1021/acs.jpca.2c07500. PMC 9805503. **^**"6.1.6: The Collision Theory". 2 October 2013.- ^
^{a}^{b}IUPAC,*Compendium of Chemical Terminology*, 2nd ed. (the "Gold Book") (1997). Online corrected version: (2006–) "steric factor". doi:10.1351/goldbook.S05998 **^**IUPAC,*Compendium of Chemical Terminology*, 2nd ed. (the "Gold Book") (1997). Online corrected version: (2006–) "collision frequency". doi:10.1351/goldbook.C01166**^**Kenneth Connors, Chemical Kinetics, 1990, VCH Publishers.**^**E.A. Moelwyn-Hughes,*The kinetics of reactions in solution*, 2nd ed, page 71.

- Introduction to Collision Theory